For the reaction $CO_{(g)} + 2H_{2(g)} \rightleftharpoons CH_3OH_{(g)}$,the true condition is:

The following equilibrium is established at $STP$. $B_{2(g)} \rightleftharpoons 2B_{(g)}$. Atoms of $B$ occupy $20 \%$ of total volume at $STP$. The total pressure of the system is $1 \ bar$. What is its $K_p$?

At $1000 \ K$,the value of $K_c$ for the reaction $A_{(g)} \rightleftharpoons B_{(g)} + C_{(g)}$ is $10 \ mol \ L^{-1}$. The value of $K_p$ (in $atm$) is: (Given $R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1}$)

$x A_{(s)} \rightleftharpoons y B_{(g)} + z C_{(g)}$. If $\frac{K_c}{K_p} = (RT)^{-2}$,then which is correct?

$1.1 \ mol$ of $A$ and $2.2 \ mol$ of $B$ are mixed in a $1 \ L$ flask until equilibrium is reached. At equilibrium,$0.2 \ mol$ of $C$ is formed. If the equilibrium reaction is $A + 2B \rightleftharpoons 2C + D$,the value of the equilibrium constant $K_C$ is:

In a $500 \ mL$ capacity vessel,$CO$ and $Cl_2$ are mixed to form $COCl_2$. At equilibrium,it contains $0.2 \ mol$ of $COCl_2$ and $0.1 \ mol$ of each of $CO$ and $Cl_2$. The equilibrium constant $K_c$ for the reaction $CO + Cl_2 \rightleftharpoons COCl_2$ is: